Agas-phase reversible reaction

a = b

is carried out under high pressure in a packed-bed reactor with pressure drop. the feed consists of both inerts i and species a with the ratio of inerts to the species a being 2 to 1. the entering molar flow rate of a is 5 mol/min at a temperature of 300 k and a concentration of 2 mol/dm^3. work this problem in terms of volume. with adiabatic operation, plot x, xe, t, and the rate of disappearance as a function of v up to v=40 dm^3. explain why the curves look the way they do. use matlab to solve the porblem.

fao = 5 mol/min

cao = 2 mol/dm^3

ci = 2 cao

cpi = 18 cal/mol/k

cpa = 160 cal/mol/k

e = 1 cal/mol

hrxn = -2 cal/mol

kc = 1000 at 300 k

cpb = 160 cal/mol/k

pb = 1.2 kg/dm^3

to = 300 k

t1 = 300 k

k1 = 0.1 1/min at 300 k

ua = 150 cal/dm^3/min/k

tao = 300 k

v = 40 dm^3

\alpha pb = 0.02 dm^3

1.consider the following balanced equation and answer parts a through. show calculations for each part.  

3 ag(s) + 4 hno3(aq) → 3 agno3(aq) + no(g) + 2 h2o(l)  

a. calculate the number of moles of agno3 produced by the reaction of 3 moles of ag with excess hno3. if the number to the left of the compound represents the number of moles of the compound which are present, then 3 moles of ag react with 4 moles hno3 to produce 3 moles agno3 (aq).

so the answer to a would be 3 moles.

b. calculate the number of moles of agno3 produced by the reaction of 108 grams of ag with excess hno3.  

i'm not sure how to plug in the grams of silver into an equation using moles to find how many moles are produced.

c. calculate the number of grams of agno3 produced by the reaction of 108 grams of ag with excess hno3  

d. calculate the number of moles of no produced as a byproduct of the reaction of 108 grams of ag with excess hno3.  

e. calculate the number of grams of no produced as a byproduct starting with 108 grams of ag and excess hno3.  

explanation: